pH and Buffer Essentials

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Core concepts of pH and buffers

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Jacquelyn Mae Adolfo

Estados Unidos

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pH and Buffer Essentials


pH and Buffer EssentialsVersión en línea Core concepts of pH and buffers por Jacquelyn Mae Adolfo 1 What is pH a measure of in a solution? a Dissolved solute strength b Water activity c Oxygen concentration d Hydrogen ion concentration 2 Which statement describes a buffer? a A mixture that resists pH change upon adding small amounts of acid or base b A solution with constant pH regardless of temperature c A substance that neutralizes all added base immediately d A compound that cannot donate or accept protons 3 Henderson–Hasselbalch equation relates pH to which factors? a pH = pKw - log([H+]) b pH = log([H+]/[OH-]) c pH = pKa + log([A-]/[HA]) d pH = pKa × [A-]/[HA] 4 What happens to buffer capacity if you double the amount of both HA and A- while keeping pH near pKa? a Buffer capacity decreases b Buffer capacity stays the same c Buffer capacity becomes zero at pKa d Buffer capacity increases 5 Which addition most strongly challenges a buffer? a Water b Strong acid or strong base c Dissolved CO2 at equilibrium d Weak acid 6 If a buffer has pKa = 7.0 and pH = 7.0, what is the ratio [A-]/[HA]? a 0:1 b 1:10 c 10:1 d 1:1 7 What is the effect of carbonic acid/bicarbonate buffer in blood? a Keeps blood pH within a narrow range (~7.35–7.45) b Never interacts with CO2 levels c Prevents any pH change completely d Raises blood pH above 9 8 Which buffer component is the conjugate base in an acetic acid buffer? a Hydrogen carbonate (HCO3-) b Sodium chloride (NaCl) c Acetate (A-) d Acetic acid (HA) 9 Why does a buffer work best near its pKa? a Because only HA matters b Because pH equals pKa only at extreme values c Because pH is far from pKa d Because [HA] and [A-] are about equal, maximizing neutralization capacity 10 What would be the immediate effect of adding a small amount of HCl to a buffered solution near its pKa? a pH would change slightly, then resist further change b No change in pH whatsoever c pH would rise dramatically d pH would jump to neutral Feedback 1 pH quantifies [H+]; acidity rises as H+ increases. 2 Buffers minimize pH changes by neutralizing added H+ or OH-. 3 The equation links pH to acid/base ratio and its pKa. 4 More total buffer species offer greater capacity to absorb added acids/bases. 5 Strong species overwhelm the buffer system, causing large pH shifts. 6 At pH = pKa, Equal concentrations of conjugate base and acid form a 1:1 ratio. 7 Blood uses the bicarbonate system to buffer CO2 produced by metabolism. 8 In an acetate buffer, HA is acetic acid and A- is acetate. 9 Maximum buffering occurs when the ratio is near 1, near pKa. 10 Buffer neutralizes some added H+, limiting pH rise, until capacity is exceeded.

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pH and Buffer Essentials

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Creada por

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pH and Buffer EssentialsVersión en línea

por Jacquelyn Mae Adolfo

What is pH a measure of in a solution?

Which statement describes a buffer?

Henderson–Hasselbalch equation relates pH to which factors?

What happens to buffer capacity if you double the amount of both HA and A- while keeping pH near pKa?

Which addition most strongly challenges a buffer?

If a buffer has pKa = 7.0 and pH = 7.0, what is the ratio [A-]/[HA]?

What is the effect of carbonic acid/bicarbonate buffer in blood?

Which buffer component is the conjugate base in an acetic acid buffer?

Why does a buffer work best near its pKa?

What would be the immediate effect of adding a small amount of HCl to a buffered solution near its pKa?

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